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The dissociation of molecular iodine into iodine atoms is represented I, (g) =21(g) At 1000.0 K, the equilibrium constant K, for the reaction is 3.80 x 10 you start with 0.0454 mol of 1, in a 2.32 L flask at 1000.0 K. What are the, concentrations of the gases at equilibrium?

The dissociation of molecular iodine into iodine atoms is represented I, (g) =21(g) At 1000.0 K, the equilibrium constant K, for the reaction is 3.80 x 10 you start with 0.0454 mol of 1, in a 2.32 L flask at 1000.0 K. What are the, concentrations of the gases at equilibrium?

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Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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The dissociation of molecular iodine into iodine atoms is represeņted I,(g) = 21(g) At 1000.0 K, the equilibrium constant K, for the reaction is 3.80 x 10 Şup you start with 0.0454 mol Of 1, in a 2.32 L flask at 1000.0 K. What are the concentrations of the gases at equilibrium? Part 1 of 2 What is the equilibrium concentration of 1,? Round your answer to 3 significant digits. M Part 2 of 2 What is the equilibrium concentration of 1? Round your answer to 3 significant digits. M
Transcribed Image Text:The dissociation of molecular iodine into iodine atoms is represeņted I,(g) = 21(g) At 1000.0 K, the equilibrium constant K, for the reaction is 3.80 x 10 Şup you start with 0.0454 mol Of 1, in a 2.32 L flask at 1000.0 K. What are the concentrations of the gases at equilibrium? Part 1 of 2 What is the equilibrium concentration of 1,? Round your answer to 3 significant digits. M Part 2 of 2 What is the equilibrium concentration of 1? Round your answer to 3 significant digits. M
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